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Chem Mr D > Bonding > Flashcards

Bonding Flashcards

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1
Q

How to make something malleable?

A

Add alloy

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2
Q

Group 2 bonding compared to group 1 bonding

A
  • stronger electrostatic force of attraction

- higher melting point

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3
Q

Metalling bonding drawing

A
  • bigger circles = bigger mass

- number in circles depends on how many electrons lost

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4
Q

What does it mean if an atom had a more positive nucleus?

A

-shells closer together so they are smaller

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5
Q

What are the 3 types of bonding?

A

Ionic
Covalent
Metallic

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6
Q

What is the nature of ionic bonding?

A

Electrostatic attraction between positive + ions

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7
Q

What is the nature of covalent bonding?

A

Shared pair of electrons between atoms

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8
Q

What is the nature of metallic bonding?

A

Attraction between lattice of positive metal ions + delocalised outer shell electrons

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9
Q

Which types of structure have ionic bonding?

A

Ionic

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10
Q

Types of structure with covalent bonding

A

Simple molecular

Giant covalent

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11
Q

Types of structure with metallic bonding

A

Metallic

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12
Q

Strength of ionic bonding

A

smaller the ions + the greater the charge on ions, the stronger attraction between positive + negative ions

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13
Q

Strength of covalent bonding

A
  • Shorter the bond, the stronger the bond
  • double bonds are stronger than single bonds
  • triple bonds stronger than double bonds
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14
Q

Strength of metallic bonds

A
  • smaller the metal ions, the greater the charge on ions

- the more delocalised outer shell electrons, the stronger the attraction between ions + electrons

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15
Q

What are the 3 types of forces between molecules?

A

Van der Waals forces
Dipole-dipole attractions
Hydrogen bonds

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16
Q

How are ions formed?

A
  • When a metal + non-metal react
  • metal atoms lose electrons to form positive ions
  • non metals gain electron to form negative ions
  • both obtain full outer shells
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17
Q

How are covalent bonds formed?

A

When non-metal + non-metal react

-the atoms share electrons so they both have full outer shells

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18
Q

What do 2 shared electrons make?

A

Single bond

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19
Q

What do 4 shared electrons make?

A

Double bond

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20
Q

What do 6 shared electrons make?

A

Triple bond

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21
Q

What is a co-ordinate (dative covalent) bond?

A

where both electrons come from the same species

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22
Q

Why are co-ordinate bonds often drawn with -> rather than - ?

A

To show the direction in which the electrons are donated

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23
Q

What happens when coordinate bonds are formed?

A

They are identical to covalent bonds

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24
Q

Sodium chloride structure bonding

A

Giant ionic lattice

Ionic bonding

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25
Q

Magnesium structure + bonding

A

Giant metallic lattice

Metallic

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26
Q

Diamond structure + bonding

A

Simple covalent molecule / tetrahedral

Covalent

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27
Q

Iodine structure + bonding

A

Simple covalent molecule

Simple covalent

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28
Q

Graphite structure bonding

A

Giant covalent lattice

Covalent

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29
Q

Ice structure + bonding

A

Regular crystal iron structure

Hydrogen

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30
Q

How many electrons can some outer shell have?

A

B 6
P 10
S 12

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31
Q

Do both the electrons have to come from different elements?

A

No
Element with 5 can share with element with 3 as 2 can come from element with 5
This is a coordinate bond

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32
Q

Shape of molecules list

A 
Linear 180
Triangular planar 120
Square planar 90
Tetrahedral 109.5
Triangular based bi pyramid 90 
Octahedral 90
33
Q

Which shapes of molecules are 3d ?

A

Tetrahedral
Triangular based bi pyramid
Octahedral

34
Q

How to use shape of molecule theory?

A 
1- central atom 
2- group (outer shell electron number)
3- charge (+ means lose electron)
4- bonds (no.of bonds)
5- total (add up 2,3,4)
6- divide by 2 (= no. of electron pairs)
7- structure (not shape)
8- look at 6+4 to see if any lone pairs 
9- shape 
10- bond angle
35
Q

What do we use electronegativity for?

A

Measure the ionic or covalent -ness of a bond

36
Q

Where to electronegativity bonds go from?

A

1 to 4

37
Q

Electronegativity definition

A

Measure of tendency of an atom to attract a Hindu f pair of elections in a covalent bond

38
Q

What is the most electronegative element?

A

Fluorine

39
Q

What 3 things determine the size of electronegativity?

A
  • size of nuclear charge (no. of protons)
  • distance between the nucleus + outer electron shell
  • shielding
40
Q

Electronegativity scale from most to least

A

Ionic
Ionic with covalent character
Covalent with ionic character
Covalent

41
Q

What happens to electronegativity if size of nuclear charge increases?

A

Increases

  • lots of protons in nucleus
  • nuclear charge size increases
  • increased attraction between nucleus + pair of electrons In covalent bond
42
Q

What happens to electronegativity when size of atom + shielding increase?

A

Decreases

  • atom size increases
  • park of electrons in covalent bond further away from nucleus
  • more shielding
  • decreases attraction from nucleus
43
Q

What is a polar bond?

A
  • if the atoms have big differences in electronegativity
  • meaning one atom holds electrons closer to itself in the bond
  • one end of bond will be slightly negative due to electrons being there
  • other end will be slightly positive due to electrons not being there
44
Q

What symbol do we used to show polarity?

A

delta negative + delta positive

45
Q

When does a non-polar covalent bond happen?

A

When 2 atoms in a covalent bond have the same electronegativity

46
Q

When does a polar covalent bond happen?

A

when two atoms in a covalent bond have a different electronegativity

47
Q

What does a non-polar covalent bond mean?

A

two electrons are shared in covalent bond

48
Q

What does polar covalent bond mean?

A

two electrons aren’t shared equally

49
Q

What happens with more electronegative atom?

A

Greater share of 2 electrons

Delta negative

50
Q

What happens with less electronegative atom?

A

Lower share of electrons

Delta positive

51
Q

Explain CO2 in terms of polar bond

A

Contains polar bonds but all dipole moments cancel out

52
Q

Explain H2O in terms of plat bonds

A

contains polar but all duplex moments don’t cancel out

53
Q

Explain CH4 In terms of polar bonds

A

no polar bonds

54
Q

What are intermolecular forces?

A

forces between molecules

55
Q

Sodium, + aluminium structure

A

giant metallic lattice

56
Q

Sodium chloride, silicon dioxide, graphite + graphene structure

A

Giant ionic lattice

57
Q

Methane, water, iodine + carbon dioxide structures

A

Simple covalent molecules

58
Q

Which structure are intermolecular forces in?

A

Simple covalent molecules

59
Q

Are intermolecular forces weaker or stronger that covalent bonds?

A

Weaker

60
Q

What are the 3 types of bonding in order of weakest to strongest?

A

Van der Waals
Dipole-dipole forces
Hydrogen bonding

61
Q

What does van der Waals bonding result in?

A

Formation of a very slight negative charge at end of the atom

62
Q

What does van der Waals bond state?

A

at any one moment there could be more electrons at one end of an atom just through chance

63
Q

What does more electrons mean in regards to van der Waals bonding?

A

More van der Waals bonding

64
Q

What can is instantaneous dipole?

A

There the other side of the atom has a very slight positive charge where there are less electrons

65
Q

What can instantaneous dipole cause?

A
  • formation of induced dipole in neighbouring atoms

- weak attractive forces between delta positive + delta negative atoms

66
Q

What must you have for dipole-dipole forces?

A

2 molecules

67
Q

What does dipole-dipole forces cause?

A
  • Attractive forces between molecules

- permanent in a molecule

68
Q

Explain HCL in terms of more dipole dipole bonding?

A

Chlorine is more electronegative than hydrogen so pulls electrons toward it

69
Q

What does some covalent bond being polar mean?

A

Means they have an electronegative elements attached to them

70
Q

Why are dipole-dipole forces not for symmetrical shape molecules?

A

Dipoles cancel eachother out

71
Q

What is a substances boiling point a measure for?

A

The intermolecular forces present between particles

72
Q

What are hydrides?

A

Elements joint to hydrogen

74
Q

What is hydrogen bonding related to?

A

Hydride boiling points

75
Q

What is hydrogen bonding?

A

The lone pair of electrons on oxygen atoms from other water molecules can interact with hydrogen
This forms a very strong intermolecular attraction called hydrogen bonding

76
Q

When does hydrogen bonding form?

A

When hydrogen is joined to nitrogen oxygen + fluorine

77
Q

What is the hydrogen bond always between?

A

The lone pair or N, F or O + H delta +

78
Q

What are some importance’s of hydrogen bonding?

A

Protein folding
DNA base pairing
Enzyme reactions

79
Q

What do noble gases + hydrides show?

A

Gradual increase in boiling points

Chem Mr D (8 decks)

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